Vista Ridge High School
6888 Black Forest Road
Colorado Springs, CO 80923
Ph: 719-494-8800 Fax: 719-494-8838
www.d49.org
Dear AP Chemistry Student & Parents,
I look forward to having you as a part of my AP Chemistry class for the 2014-2015 school year. This letter contains
information that pertains to your AP Chemistry Summer assignment. Each of the following must be completed. AP
Chemistry is a fast-paced course that begins with new material in the very first week. This assignment must be completed
so that you do not fall behind at the very beginning of the course.
We will have a summer assignment quiz on the first
day of class.
As difficult as AP Chemistry is, you will find that it will never be easier to learn College Freshman-level
Chemistry than it is now! There are several reasons for this:
a) High school classes are generally smaller than college classes. It is not unusual for freshman college classes to
have 200 or more students! In this situation, it is nearly impossible to ask a question during class or get any individual
attention after class. In AP Chemistry, we always take time for questions and answers, and I am almost always available
for after school help – and often on weekends and breaks too!
b) Many college professors don't regard teaching Freshman Chemistry as a priority for their job – many
concentrate on their research, and consider teaching to be an interruption and distraction to that end. In extreme cases,
a college instructor may not speak English such that it can be easily understood. At our school, teaching is our Number
1 priority and we do it well!
c) At times Freshman Chemistry is used to "weed out" students. Most colleges prefer not to have large class
sizes in their upper division courses. Therefore the grades and difficulty level of the freshman courses are adjusted so
that only small numbers of very outstanding students will be able to move on. This can result in a large portion of
students in freshman chemistry flunking the course! At our school we don't have these kinds of pressures, and all
students are encouraged to become successful.
d) AP Chemistry will teach you to think at higher levels. Learning will rarely be of the "parrot-back" variety (ie.
where the teacher gives a lecture, and the student is expected to give back the same information on a test-similar to a
parrot!) In AP Chemistry, you will be forced to think and apply concepts to new situations, and even derive your own
theories from application. This is excellent preparation for the higher levels of thinking required in college.
Students need to be realistic about the expectations for this course. Many students THINK they are ready for
college level work, but really don't know what that means. In order to get a more realistic view of this course, I have
included some perceptions entering students have, and the reality of the situation:
1) PERCEPTION: I have always been a "straight A" student, and always will be.
REALITY: AP Chemistry can mean death to a 4.0 grade point average. Although there are several "A" 's (about
one fourth of the class), there are also "B"’s, "C"’s, "D"’s and "F"‘s. And all of these students were top students in their
First Year Chemistry class!!! If your main purpose in taking this class is to collect one more "A", you are taking the class
for the wrong reason, and may be disappointed. There are easier classes to get an "A" in.
2) PERCEPTION: I can miss class (sports, activities, family vacations, jobs, field trips etc.) and catch up on my own. I
always have before.
REALITY: You can’t! In AP Chemistry, you have to give up a lot to get a lot. Missing class is the number one reason
why students fall behind, get lost, give up, and either drop the class, or get a low grade. You CANNOT be gone for
three days, and expect to get caught up with a 10 minute session after school. I cannot teach in 10 minutes what it took 3
hours to teach earlier! (Amazingly, some students do expect that!!!) You cannot expect to just “figure it out for yourself”
or get help from a friend – the material is just too difficult. Therefore you will have to say "no" to things that will take you
out of class such as field trips, band trips, student council, and the multitude of other "excuses" for missing class. Families
are asked to take vacations during school holidays only. You have GOT to get to a college level of maturity where even
though you have a legal excuse to miss class, you choose not to.
3) PERCEPTION: Like all teachers, Mrs. Maze is exaggerating about how much work there is, and how tough it
really is.
REALITY: I’m not exaggerating! Probably the best way to check this is to talk with students who have taken the class
before. I can provide you with a list if you wish.
4) PERCEPTION: Mrs. Maze is making this class a lot tougher than it really needs to be.
REALITY: Never forget, this is a college level course, NOT an advanced high school course! If I am doing my job,
students in this course should learn as much as they would if they were taking freshman chemistry at any college or
university in the United States. From feedback I have received from former students, that goal is being achieved. A
second goal is to properly prepare students for the AP Exam in May. I cannot make the course easier and still
accomplish these goals. Every former student who has taken freshman college chemistry has found that (s)he had a
tremendous advantage over other students. I have NEVER had former students come back and say they wish I hadn't
made it so tough!
5) PERCEPTION: If the majority of the class falls behind, Mrs. Maze will just have to slow down so that we can
catch up.
REALITY: I can’t! You will find that time is of the essence in this course. As much as I may like to and as much as the
students may need it, our schedule cannot be adjusted to accommodate those who cannot keep up. Students will be
expected to study the text on their own, and class time will be used more for clearing up questions than for introducing
new material. There is really no other way to cover the vast amount of material required by the AP exam. If we slow down
to make the course easier, or allow students to catch up, we will not cover the required subject matter, and students will
have to face exam questions on material not covered. As a result, I will make a schedule that will allow us to complete all
requirements prior to the exam, and students MUST keep to this schedule. Chemistry topics build on each other, and
students who get behind have a (nearly) impossible task in catching up. Students can expect to spend about one hour
outside of class time just in the study of chemistry each night, including the weekends. Certainly any students who have
after-school jobs, or who are heavily involved in after-school activities, will have to budget their time very carefully.
6) PERCEPTION: All this work Mrs. Maze is talking about must be just for the "dummies". I'm smarter than that!
REALITY: All students who are successful in this course will have to spend time in class after school, either getting
help on an assignment, completing lab work, or reviewing for tests. If you are NEVER available immediately after school
to do chemistry work, you should not take this course. Occasionally labs will require us to meet 30 – 60 minutes after
school gets out (4th Block AP Chem) in order to have a two-hour lab block. If you are unable to make this commitment,
you will not be able to take this course. Late-comers for lab will NOT be admitted to the room for safety reasons. I am
often available for help before school or during lunch, and almost every day after school. We also form study groups that
meet on Saturdays at Starbucks or at school, especially when there are Monday holidays built in to the school
calendar. Students will be encouraged to form their own study groups to get many of their questions answered.
7) PERCEPTION: Mrs. Maze doesn't really expect us to do a summer assignment, and she isn't really going to give
us a test the first day of class in August.
REALITY: I am serious about this - just ask students who have already taken the course. The summer assignment is
mainly a review of first year Chemistry. The test will encourage you to do most of the memorization for the course before
the school year begins. This early work will allow us to spend more time later on more difficult topics. You will find the
summer assignment and the review for the "first day test" at the end of this letter.
Now that I have scared all of you, I will say that there is fun to be had in this course, as well as the satisfaction of
challenging yourself to the limit of your academic ability. We have a creative way of providing donuts for the early
morning lab sessions, and in the past we have had class field trips and parties. I hope you have a great summer-don't
forget your summer assignment/first day test- and I'll see you in the fall!
1.
Check out an AP Chemistry Book from the library BEFORE THE END OF THE SCHOOL
YEAR! You will need this for the reading assignment in July.
2.
Please complete this form online http://goo.gl/forms/sSrLrZF3ry so I can get in touch with you over the summer
and throughout the school year if necessary.
3.
Memorize Formulas, Charges, and Names for all of the Ions given on the handout. The list includes both the
polyatomic and monatomic ions. Make sure that you know names and formulas. Also, for the monatomic ions make
sure you know both the stock and classical names. You must know how to write correct chemical formulas using these
ions.
4.
Memorize Solubility Rules for the Soluble and Insoluble Ionic Compounds. You need to be able to look at the
formula for a compound and know if that compound will be soluble or insoluble in a solution.
5.
Memorize Formulas and Common Names for the Certain Acids and Compounds:
a.
Hydrochloric Acid – HCl
b.
Sulfuric Acid – H2SO4
c.
Phosphoric Acid – H3PO4
d.
Acetic Acid – HC2H3O2
e.
Carbonic Acid – H2CO3
f.
Nitric Acid – HNO3
g.
AlK(SO4)2·12H2O alum
h.
CH4 methane
i.
C6H6 benzene
j.
C10H8 naphthalene (mothballs)
k.
CHCl3 chloroform
l.
CH3OH methyl alcohol or methanol
(wood alcohol)
m. C2H5OH ethyl alcohol or ethanol
(drinking alcohol)
n.
CH3COCH3 acetone
o.
C3H5(OH)3 glycerin
p.
C6H8O6 L-ascorbic acid (vitamin C)
q.
CaCO3 chalk, marble, limestone
r.
CaO quicklime
s.
Ca(OH)2 slaked lime (lime water)
t.
CaSO4 gypsum, plaster of paris
u.
Fe3O4 or Fe2O3 rust
v.
HCHO formaldehyde
w. H2O water
x.
Hg quicksilver
y.
K2CO3 potash
z.
MgO magnesia
ff. NaHCO3 baking soda
aa. MgSO4 epsom salts
gg. NaNO3 saltpeter
bb. NH3 ammonia
hh. NaOCl bleach
cc. N2O laughing gas
ii.
NaOH caustic soda or lye
dd. Na2CO3 soda ash
jj.
SiO2 sand, quartz
ee. NaCl table salt
6.
Mid- July: Outline Chapters 1 & 2 in your textbook and complete the AP Chemistry Summer Assignment
Worksheet to make sure that you are ready for the quiz on our first day.
You will have a quiz on the first day of class when you return from break. Please do not put this assignment off until the
last minute. You will not be able to get it done. A failing grade on this test will tell me that you are not ready to do the
work necessary in AP Chemistry and you will be asked to attend mandatory tutoring for the first two weeks of the
semester. Please do not hesitate to contact me if you have any questions. I can be reached by e-mail or phone. Thank
you in advance for your cooperation and hard work. I look forward to having you in class! It will be a blast…sometimes
quite literally!
Sincerely,
Jennifer Maze
w: (719)494-6888 x 2259,
c: (719)469-0383 (text),
jmaze@d49.org
Follow on Twitter @JenGrayScience and/or @VRAPChem
Chemistry Study Sheet: Ions and Prefixes
Element
Aluminum
Barium
Cadmium
Calcium
Cesium
Chromium(II)/Chromous
Chromium(III)/Chromic
Cobalt(II)/Cobaltous
Cobalt(III)/Cobaltic
Copper(I)/Cuprous
Copper(II)/Cupric
Gold
Hydrogen
Iron(II)/Ferrous
Iron(III)/Ferric
Lithium
Ammonium
Hydronium
Monatomic Cations
Formula
Element
Al3+
Lead(II)/Plumbous
Ba2+
Lead(IV)/Plumbic
Cd2+
Maganese(II)/Manganous
Ca2+
Maganese(III)/Manganic
Cs+
Magnesium
Cr2+
Mercury(I)/Mercurous
Cr3+
Mercury(II)/Mercuric
Co2+
Nickel (II)/Nickelic
Co3+
Potassium
Cu+
Rubidium
Cu2+
Silver
Au+
Sodium
H+
Strontium
Fe2+
Tin(II)/Stannous
Fe3+
Tin(IV)/Stannic
Li+
Zinc
Formula
Pb2+
Pb4+
Mn2+
Mn3+
Mg2+
Hg22+
Hg2+
Ni2+
K+
Rb+
Ag+
Na+
Sr2+
Sn2+
Sn4+
Zn2+
Molecular Compounds
1= mono
2 = di
3 = tri
4 = tetra
5 = penta
6 = hexa
7 = hepta
8 = octo
9 = nano
10 = deca
**Drop Double Vowels
Polyatomic Cations
NH4+
H3O+
Monatomic Anions
Element
Formula
Hydride*
HFluoride*
FChloride*
ClBromide*
BrIodide*
IOxide*
O2Sulfide
S2Nitride*
N3*Exists as diatomic molecules
Naming Acids
Monatomic Anion
*Name starts with hydroIon has –ic at the end and add
“acid”
Polyatomic Anion
*No hydro in name
If ion ends in –ite change it to
–ous and add “acid”
If ion ends in –ate change it to –ic
and add acid
Remember: “I –ate something –
icky”
Name
Aresenate
Borate
Bromate
Carbonate
Chlorate
Chlorite
Chromate
Cyanide
Dichromate
Dihydrogen Phosphate
Polyatomic Anions
Formula
Name
AsO43Hypochlorite
BO33Iodate
BrO3Nitrate
CO32Nitrite
ClO3Oxalate (ethanedioate)
ClO2Perchlorate
CrO42Permanganate
CNPeroxide
Cr2O72Phosphate
H2PO4-
Formula
ClOIO3NO3NO2C2O42ClO4MnO4O22PO43-
Phosphite
PO33-
Silicate
SiO32-
Sulfate
SO42-
Hydrogen Carbonate (bicarbonate)
CH3CO2-or
C2H3O2HCO3-
Hydrogen Phosphate (biphosphate)
HPO42-
Sulfite
SO32-
Hydrogen Sulfate (bisulfate)
Hydroxide
HSO4OH-
Tetraborate
Thiocyanate
B4O72SCN-
Thiosulfate
S2O32-
Ethanoate
**Hydrate (combine w prefix)
H2O
Solubility Rules
Circle all the ionic compounds that are INSOLUBLE (these are the precipitates)
Name ONE or more compounds in each row
MgF2
CuSO4
NH4Cl
Fe(OH)3
CsF
AgCl
CdS
CuF2
PbSO4
Ba(OH)2
Na2SO4
NH4OH
Sr(NO3)2
Hg2I2
Na2CrO4
BaCO3
PbBr2
CaC2O4
HC2H3O2
MgO
AP Chemistry Summer Assignment
The following assignment is to be completed and brought with you on the first day of class.
Nomenclature
Name the following binary compounds
1.
IF7
4.
N2O4
7.
PCl3
2.
N2O5
5.
As4O10
8.
S2Cl2
3.
XeF2
6.
SF6
Name these binary compounds with a fixed charge metal.
9.
12. KI
15. CaF2
10. MgO
AlCl3
13. SrBr2
16. Al2O3
11. BaI2
14. Na2S
Name these binary compounds of cations with variable charge.
17. CuCl2
20. PbCl4
23. AuI3
18. Fe2O3
21. Cu2S
24. CoP
19. SnO
22. HgS
Name these compounds with polyatomic ions.
25. Fe(NO3)3
28. Ca(ClO3)2
31. NH4NO2
26. NaOH
29. KNO2
32. Cu2Cr2O7
27. Cu2SO4
30. NaHCO3
Name these binary acids
33. HCl
34. HI
35. HF
Name these acids with polyatomic ions.
35. HClO4
38. H3PO4
41. H2C2O4
36. H2SO4
39. HNO2
42. H2CO3
37. HC2H3O2
40. H2CrO4
Name these compounds appropriately.
43. CO
48. OF2
53. CuCr2O7
44. NH4CN
49. LiMnO4
54. K2O
45. HIO3
50. HClO
55. FeF3
46. NI3
51. HF
56. KC2H3O2
47. AlP
52. SO2
57. MnS
58. Tin (IV) phosphide
62. Sulfurous acid
66. Gallium arsenide
59. Copper (II) cyanide
63. Lithium silicate
67. Cobalt (II) chromate
60. Magnesium hydroxide
64. Potassium nitride
68. Zinc fluoride
61. Sodium peroxide
65. Chromium (III) carbonate
69. Dichromic acid
Write the formulas.
Solubility rules
Review solubility rules and identify each of the following compounds as soluble or insoluble in water.
70. Na2CO3
73. K2S
76. AgI
71. CoCO3
74. BaSO4
77. Ni(NO3)2
72. Pb(NO3)2
75. (NH4)2S
78. KI
79. FeS
80. PbCl2
81. CuSO4
Predict whether each of these double replacement reactions will give a precipitate or not based on the solubility of the
products. If yes, identify the precipitate.
88. silver nitrate and potassium chloride
89. magnesium nitrate and sodium carbonate
90. strontium bromide and potassium sulfate
91. cobalt (III) bromide and potassium sulfide
92. ammonium hydroxide and copper (II) acetate
93. lithium chlorate and chromium (III) fluoride
Balancing Equations
Balance the following equations with the lowest whole number coefficients.
94. S8 +
O2  SO3
95. C10H16 + Cl2 
96. Fe +
O2 
C +
98. KClO3 
HCl
Fe2O3
97. C7H6O2 + O2  CO2 + H2O
99. H3AsO4 
KCl + O2
As2O5 + H2O
100. V2O5 + HCl  VOCl3 +
H2O
101. Hg(OH)2 + H3PO4  Hg3(PO4)2 + H2O
Stoichiometry and Limiting Factor
102. Given the equation below, what mass of water would be needed to react with 10.0g of sodium oxide?
Na2O + H2O  2NaOH
103. What mass of sodium choride is formed along with 45.0g of oxygen gas?
2NaClO3  2NaCl + 3O2
104. What mass of water will be produced when 100.0g of ammonia is reacted with excess oxygen?
4NH3 + 5O2  4NO + 6 H2O
105. If the reaction in #104 is done with 25.0g of each reactant, which would be the limiting factor?
106. Na2S + 2AgNO3  Ag2S + 2NaNO3
a. If the above reaction is carried out with 50.0g of sodium sulfide and 35.0g of silver nitrate, which is the limiting factor?
b. What mass of the excess reactant remains?
c. What mass of silver sulfide would precipitate?
107. What volume of hydrogen gas (measured at STP) would result from reacting 75.0g of sodium hydroxide with 50.0g of
aluminum?
6NaOH + 2Al  2Na3AlO3 + 3H2